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75.0 g
A balanced equation for the reaction is 2 KClO3 -> 2 KCl + 3 O2. Therefore, each mole of potassium chlorate produces 3/2 moles of oxygen, and 1.2 moles of potassium chlorate produces (3/2)1.2 or 1.8 moles of oxygen.
For every mole of KClO3 decomposed, three moles of O2 are produced. So, 1.2 moles of KClO3 would produce 3.6 moles of O2.
10 mol KClO3 * 3mol O/ 1 mol KClO3= 30
A mole of any element, compound, etc is defined by Avogadro's Constant. There are always 6.02214179×1023 atoms in one mole of that substance.
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How many moles of potassium chlorate must be used to produce 6 moles of oxygen gas?
2KClO3 --> 2KCl + 3O2For every 3 moles of oxygen gas produced, 2 moles of potassium chlorate are used.6 moles O2 * (2 moles KClO3 reacted / 3 moles O2 produced) = 4 moles KClO3
A How many moles of O2 were produced b What percent of the mixture was KClO3 and KCl?
a) To find the number of moles of O2 produced, you would need the balanced chemical equation for the reaction involving KClO3 and KCl. Once you have that, you can use stoichiometry to determine the number of moles of O2 formed. b) The percentage of the mixture that is KClO3 and KCl can be calculated by dividing the mass of each component by the total mass of the mixture and then multiplying by 100 to express it as a percentage.
When 40 grams of ammonium nitrate explode 14 grams of nitrogen and 8 grams of oxygen form how many grams of water form?
To calculate the grams of water formed, we first need to determine the moles of nitrogen and oxygen produced. Using the given data, we find that 14 grams of nitrogen is equivalent to 1 mole and 8 grams of oxygen is also equivalent to 0.5 moles. In the explosion, these moles of nitrogen and oxygen will combine with hydrogen to form water. Since the molar ratio of hydrogen to nitrogen and oxygen is 2:1, the moles of water produced will be 1 mole (from nitrogen) + 0.5 moles (from oxygen) = 1.5 moles. Finally, converting moles to grams, 1.5 moles of water is equal to 18 grams. Thus, 18 grams of water would form during the explosion.
Calculate the number of moles of oxygen atom in 18.1 mole of CH2O?
Since there is only 1 oxygen atom in CH2O, there is the same amount of oxygen atoms as there are molecules of CH2O. So the answer is 18.1 mole. But if you burn it, you will form oxygen in its natural form, which is O2. So there will only be the half the amount of the oxygen. Then the answer would be 18.1 / 2 = 9.05 mole.
How many grams of oxygen are in 5.75 moles of aluminum oxide?
To determine the number of grams of oxygen in 5.75 moles of aluminum oxide, you first need to know the molar ratio of oxygen to aluminum oxide. In aluminum oxide (Al2O3), there are 3 oxygen atoms for every 2 aluminum atoms. 5.75 moles of Al2O3 would contain 5.75 moles * 3 moles of O / 2 moles of Al2O3 = 8.63 moles of oxygen. Finally, calculate the mass of 8.63 moles of oxygen using its molar mass of 16 g/mol. Therefore, 5.75 moles of aluminum oxide would contain 8.63 moles * 16 g/mol = 138 grams of oxygen.
How many moles of potassium chlorate must be used to produce 6 moles of oxygen gas?
2KClO3 --> 2KCl + 3O2For every 3 moles of oxygen gas produced, 2 moles of potassium chlorate are used.6 moles O2 * (2 moles KClO3 reacted / 3 moles O2 produced) = 4 moles KClO3
How many moles of oxygen are produced when 7.5 moles of potassium chlorate decompose completely?
For every mole of potassium chlorate that decomposes, three moles of oxygen are produced. Therefore, if 7.5 moles of potassium chlorate decompose, 22.5 moles of oxygen would be produced (7.5 moles x 3).
How many moles of KClO3 on decomposition give 1 mole of oxygen?
2 grams of Oxygen can be obtained from 5 grams of KClO3 (only if the "CL" means "Cl", which is Chlorine! Remember that only the first letter of the atomic symbol is capitalized.)
A How many moles of O2 were produced b What percent of the mixture was KClO3 and KCl?
a) To find the number of moles of O2 produced, you would need the balanced chemical equation for the reaction involving KClO3 and KCl. Once you have that, you can use stoichiometry to determine the number of moles of O2 formed. b) The percentage of the mixture that is KClO3 and KCl can be calculated by dividing the mass of each component by the total mass of the mixture and then multiplying by 100 to express it as a percentage.
2 H2 plus O2 2 H2O - How many moles of water will be produced from a fuel cell that consumes 0.633 moles of oxygen?
For every mole of oxygen consumed in the reaction 2H2 + O2 -> 2H2O, two moles of water are produced. Therefore, if 0.633 moles of oxygen are consumed, the number of moles of water produced would be 2 x 0.633 = 1.266 moles.
How many moles of oxygen will be produced from the complete combustion of 4 moles of propane?
The balanced chemical equation for the combustion of propane is: C3H8 + 5 O2 -> 3 CO2 + 4 H2O. This means that 5 moles of oxygen are required to completely combust 1 mole of propane. Therefore, 20 moles of oxygen would be produced from the complete combustion of 4 moles of propane.
What is the grams of substance in 2 moles of KClO3?
Alls you do to find a molar mass is add up all of the atomic masses. Potassium=39.09 Chlorine= 35.453 Oxygen(3)=15.999. So KClO3 would equal 271.65g to a mol? Then I think to find the number of atoms of each you would take the atomic mass * avacodo's number so it would be for example chlorine. 1gCl(35.453/1)(6.022*10^23/1) However I might be wrong on that part.
If 4.8g of oxygen gas is completely converted to ozone how many molecules of ozone would be produced?
4.8/16 moles of oxygen atoms converts to 1.6/16 moles of ozone molecules.
In the reaction 2CO plus O2 equals 2CO2 what is the ratio of moles of oxygen used to moles of CO2 produced?
The ratio is 1:2. For every 1 mole of O2 consumed, 2 moles of CO2 are produced in this reaction.
When 36.3 g of potassium chlorate is heated 22.1 g of potassium chloride is produced What mass of oxygen is produced?
Equation: 2KClO3 + Cl2 ---> 2KCl + 3O2 + Cl2 1. Solve for the number of moles of KClO3 in 36.3 g. (.2962 molKClO3) 2. Multiply that value by (3/2), from the equation's coefficients. (.4447 molO2) Note: A BCA table could also be used. 3. Solve for the mass of .4447 molO2. 14.2 grams of oxygen would be produced.
How many moles of SO3 would be produced when 1.2 moles of oxygen is consumed in the equation S plus O2 equals SO3?
Since the equation provided is 2S + 3O2 → 2SO3, it can be seen that 3 moles of O2 are required to produce 2 moles of SO3. Therefore, with 1.2 moles of O2 consumed, the moles of SO3 produced would be (1.2 moles O2) x (2 moles SO3 / 3 moles O2) = 0.8 moles of SO3.
How many moles of Co2 will be produced from the reaction of three moles of acetylene with excess oxygen?
Since acetylene (C2H2) has a stoichiometry of 2 moles of acetylene to produce 2 moles of CO2, three moles of acetylene would produce 3 moles of CO2. The reaction with excess oxygen ensures that all the acetylene is fully converted to CO2.
